Calculate the vapor pressure of absolute ethyl alcohol at 25 ºC. ΔHvap = 39.3 kJ/mol; normal boiling point = 78.3 ºC.
Calculate the vapor pressure of absolute ethyl alcohol at 25 ºC. ΔHvap = 39.3 kJ/mol; normal...
17. The normal boiling point of acetone is 56.2 oC and its ΔHvap is 25.5 kJ/mol. At what temperature does acetone have a vapor pressure of 375 mmHg?
a.) Determine the normal boiling point of a substance whose vapor pressure is 55.1 mm Hg at 35°C and has a ΔHvap of 32.1 kJ/mol. b.) Determine the vapor pressure (in mm Hg) of a substance at 29°C, whose normal boiling point is 76°C and has a ΔHvap of 38.7 kJ/mol. c.) Which of the temperatures below is most likely to be the boiling point of water at 880 torr? 100°C 92°C 105°C 88°C
ethyl alcohol has a vapor pressure of 20 mmHg at 8.0 C and a normal boiling point of 78.4 C. estimate the vapor pressure at 45 C using (a) the Antoine equation. (b) the Clausius-Clapeyron equation and the two given data points; and (c) linear interpolation between the two given points. taking the 1st estimate to be correct, calculate the percentage error associated with the second and third estimates.
The ΔHvap of hexane is 28.16 kJ/mol and its boiling point is 65.2 °C. Using the Clausius-Clapeyron equation, calculate the vapor pressure (mm Hg) of hexane at 25.0 °C.
Diethyl ether has a ΔHvap of 29.1 kJ/mol and a vapor pressure of 0.703 atm at 25.0°C. What is its vapor pressure at 82.0°C?
What is the normal boiling point of a substance whose vapor pressure is 67.1 mm Hg at 47°C and has a ΔHvap of 46.2 kJ/mol.
The vapor pressure of ethanol is 1.00 x 102 mmHg at 34.90oC. What is its vapor pressure at 51.73 oC? (ΔHvap for ethanol is 39.3 Kj/mol.) Given the vapor pressure at one temperature, P1, we can calculate the vapor pressure at a second temperature, P2. In (P1/P2) = ΔHvap/R (1/T2 - 1/T1) Where, ΔHvap for ethanol must have the units of J/mol. R = 8.314 J/K.mol .. The temperatures must be in Kelvins. Solve for P2, What is the vapor...
A certain liquid has a vapor pressure of 92.0 Torr92.0 Torr at 23.0 ∘C23.0 ∘C and 332.0 Torr332.0 Torr at 45.0 ∘C.45.0 ∘C. Calculate the value of ΔH∘vapΔHvap∘ for this liquid. ΔH∘vap=ΔHvap∘= kJ/molkJ/mol Calculate the normal boiling point of this liquid. boiling point
The vapor pressure of ethanol is 1.00 × 102 mmHg at 34.90°C. What is its vapor pressure at 52.89°C? (ΔHvap for ethanol is 39.3 kJ/mol.)
196 The normal boiling point of Br2(l) is 58.8 ∘C, and its molar enthalpy of vaporization is ΔHvap = 29.6 kJ/mol. a) When Br2(l) boils at its normal boiling point, does its entropy increase or decrease? b) Calculate the value of ΔS when 1.50 mol of Br2(l) is vaporized at 58.8 ∘C. ΔS= (answer in J/K)